A chemistry Lab- incharge kept Zn metal in `FeSO_4`solution and observed that after some time green `FeSO_4` solution turn to colourless and some brown powder was deposited on zinc. In the above section, zn metal acted as

Options

A. oxidising agent
B. reducing agent
C. dehydrating agent
D. catalyst

Answer

To solve the question, we need to analyze the reaction that occurs when zinc (Zn) is placed in a solution of iron(II) sulfate (FeSO₄).

### Step 1: Identify the Reactants
- The reactants in this case are zinc metal (Zn) and iron(II) sulfate solution (FeSO₄).

### Step 2: Observe the Changes
- Initially, the FeSO₄ solution is green due to the presence of Fe²⁺ ions.
- After some time, the solution turns colorless, indicating that the Fe²⁺ ions are being reduced to Fe³⁺ ions or possibly being displaced from the solution.
- A brown powder is deposited on the zinc, which is likely iron (Fe) that has been displaced from the solution.

### Step 3: Determine the Reaction
- Since zinc is more reactive than iron, it can displace iron from its salt solution. The reaction can be represented as:
\[ \text{Zn (s)} + \text{FeSO}_4 (aq) \rightarrow \text{ZnSO}_4 (aq) + \text{Fe (s)} \]
- In this reaction, zinc is oxidized to Zn²⁺ ions, while iron ions (Fe²⁺) are reduced to solid iron (Fe).

### Step 4: Identify the Role of Zinc
- In this reaction, zinc donates electrons to iron ions, which means it is acting as a reducing agent because it reduces the iron ions while itself being oxidized.

### Conclusion
- Therefore, in the above situation, zinc metal acted as a **reducing agent**.

### Final Answer
Zinc metal acted as a **reducing agent**.

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